Consider the equilibrium between COBr2, CO and Br2. COBr2(g) <-->CO(g) + Br2(g) K = 2.08 at...

Consider the equilibrium between COBr₂, CO and Br₂.

COBr₂(g) <-->CO(g) + Br₂(g) K = 2.08 at 382 K

The reaction is allowed to reach equilibrium in a 14.6-L flask. At equilibrium, [COBr₂] = 4.50×10^-2 M, [CO] = 0.306 M and [Br₂] = 0.306 M.
(a) The equilibrium mixture is transferred to a 7.30-L flask. In which direction will the reaction proceed to reach equilibrium? right or left

(b) Calculate the new equilibrium concentrations that result when the equilibrium mixture is transferred to a 7.30-L flask.

[COBr₂]	=	M
[CO]	=	M
[Br₂]	=	M

Solutions

Expert Solution

queen_honey_blossom answered 6 months ago

Next > < Previous

Related Solutions

Given the following reactions: COBr2 (g) --------------- > CO (g) + Br2 (g) K = .190...

Given the following reactions: COBr2 (g) --------------- > CO (g) + Br2 (g) K = .190 at 73 °C 2 BrCl (g) ------------ > Br2 (g) + Cl2 (g) K = 310 at 73 °C (estimated) Find the equilibrium constant at 73 °C for: CO + BrCl ------- > COBr2 + Cl2

A proposed mechanism for the preparation of COBr2 from CO(g) and Br2 is: Br2 ⇄ 2...

A proposed mechanism for the preparation of COBr2 from CO(g) and Br2 is: Br2 ⇄ 2 Br (g) fast Br(g) + CO (g) ⇄ COBr fast COBr + Br2 → COBr2 + Br slow The correct rate law for this mechanism is: A. k [CO][Br2] B. k [CO] / [Br2]1/2 C. k[Br2] D. k [CO]2[Br2] E. k [CO][Br2]3/2

Carbonyl bromide, COBr2, decomposes to CO and Br2 with and equilibrium constant of Kc of 0.190...

Carbonyl bromide, COBr2, decomposes to CO and Br2 with and equilibrium constant of Kc of 0.190 at 73C. COBr2(g) <--> CO (g) + Br2 (g) if 0.015 mol COBr2 is in a 2.50 L flask at equilibrium, what are the concentrations of CO and Br2 at equilibrium?

Consider the following equilibrium: 2NOBr(g) <------> 2NO(g) + Br2(g). An equilibrium mixture is 0.146 M NOBr,...

Consider the following equilibrium: 2NOBr(g) <------> 2NO(g) + Br2(g). An equilibrium mixture is 0.146 M NOBr, 0.270 M NO, and 0.236 M Br2. a) What is the value of Kc at the temperature of the above concentrations? b) How many moles/liter of NOBr must be added to the above equilibrium mixture to produce an equilibrium mixture that is 0.439 M Br2? c) If the temperature is 370 K, what is the value of Kp? d) What is the value of...

Consider the equilibrium N2(g) + O2(g) ⇄ 2 NO(g) At 2300 K the equilibrium constant K...

Consider the equilibrium N2(g) + O2(g) ⇄ 2 NO(g) At 2300 K the equilibrium constant K = 1.7 × 10-3. Suppose that 0.0150 mol NO(g), 0.250 mol N2(g), and 0.250 mol O2(g) are placed into a 10.0-L flask and heated to 2300 K. The system is not at equilibrium. Determine the direction the reaction must proceed to reach equilibrium and the final equilibrium concentrations of each species. to the right to the left [N2] =____ mol/L [O2] = ____mol/L [NO]...

Consider the following equilibrium: 2NOBr(g) 2NO(g) + Br2(g) An equilibrium mixture is 0.150 M NOBr, 0.395...

Consider the following equilibrium: 2NOBr(g) 2NO(g) + Br2(g) An equilibrium mixture is 0.150 M NOBr, 0.395 M NO, and 0.221 M Br2. a) What is the value of Kc at the temperature of the above concentrations? Kc = M b) How many moles/liter of NOBr must be added to the above equilibrium mixture to produce an equilibrium mixture that is 0.448 M Br2? mol/L NOBr must be added c) If the temperature is 400 K, what is the value of...

Consider the equilibrium N2(g)+O2(g)+Br2(g)⇌2NOBr(g) Part A Calculate the equilibrium constant Kp for this reaction, given the...

Consider the equilibrium N2(g)+O2(g)+Br2(g)⇌2NOBr(g) Part A Calculate the equilibrium constant Kp for this reaction, given the following information (at 295 K ): 2NO(g)+Br2(g)⇌2NOBr(g)Kc=2.1 2NO(g)⇌N2(g)+O2(g)Kc=2.2×1030 Express your answer using two significant figures.

Consider the reaction: CO(g) + H2O(g)<------> CO(g) + H2(g) and K = 0.118 at 4000 K....

Consider the reaction: CO(g) + H2O(g)<------> CO(g) + H2(g) and K = 0.118 at 4000 K. A reaction mixture initially contains a CO partial pressure of 1344 mbar and a H2O partial pressure of 1766 mbar at 4000K. Calculate the equilibrium partial pressures of each of the products.

Consider the following equilibrium: CO2(g) + H2(g)---CO(g) + H2O(g); Kc = 1.6 at 1260 K Suppose...

Consider the following equilibrium: CO2(g) + H2(g)---CO(g) + H2O(g); Kc = 1.6 at 1260 K Suppose 0.038 mol CO2 and 0.022 mol H2 are placed in a 1.50-L vessel at 1260 K. What is the equilibrium partial pressure of CO(g)? The answer is either 9.9 atm or 1.1 atm. But my question is WHY IS ONE CHOICE INCORRECT since I get both in my calculations.

Consider the following equilibrium for which H = 16.48: 2 NOBr(g) Y--> 2 NO(g) + Br2(g)...

Consider the following equilibrium for which H = 16.48: 2 NOBr(g) Y--> 2 NO(g) + Br2(g) How will each of the following changes affect an equilibrium mixture of the 3 gases in this reaction? (a) NO is added to the system. (b) The reaction mixture is heated. (c) The volume of the reaction vessel is doubled. (d) A catalyst is added to the reaction mixture. (e) The total pressure of the system is increased by adding a noble gas. (f)...

Subjects